Answer
$\Delta _{r}G^{\circ}=46.5\,kJ/mol\gt0$
This reaction is not product-favored.
Work Step by Step
$\Delta_{r}G^{\circ}=\Delta _{r}H^{\circ}-T\Delta _{r}S^{\circ}$
$=52.96\,kJ/mol-(25+273)K(21.81\,JK^{-1}mol^{-1})$
$=52.96\,kJ/mol-(298\,K)(0.02181\,kJK^{-1}mol^{-1})$
$=46.5\,kJ/mol$
$\Delta_{r}G^{\circ}$ is positive.
$\implies$ The reaction is reactant-favored.
